BIO-CHEMISTRY FINAL EXAM || 100 QUESTIONS AND
CORRECT DETAILED ANSWERS LATEST UPDATE 2025
GRADED A+
For which reaction will Kp = Kc?
a. CaCO3 (s) ↔ CaO (s) + CO2 (g)
b. 2 H2O (l) ↔ 2 H2 (g) + O2 (g)
c. 2 HgO (s) ↔ Hg (l) + O2 (g)
d. S (s) + O2 (g) ↔ SO2 (g)
e. H2CO3 (s) ↔ H2O (l) + CO2 (g) -ANSWER: S (s) + O2 (g) ↔ SO2 (g)
For the following example, identify the following.
H2O (l) → H2O(g)
A.a positive ΔH and a positive ΔS
B. a positive ΔH and a negative ΔS
C. a negative ΔH and a positive ΔS
D. a negative ΔH and a negative ΔS
E. It is not possible to determine without more information. -ANSWER: a positive ΔH and a
positive ΔS
What is Δn for the following equation in relating Kc to Kp?
CH4(g) + H2O(g) ↔ CO(g) + 3 H2(g)
A. -1
B. -2
C. 3
,D. 1
E. 2 -ANSWER: 2
The reaction below has a Kp value of 41. What is the value of Kc for this reaction at 400 K?
N2(g) + 3 H2(g) ↔ 2 NH3(g)
A. 41
B. 4.4 × 10^(4)
C. 1.9 × 10^(4)
D. 2.4 × 10^(-2)
E. 2.3 × 10^(-5) -ANSWER: 4.4 × 10^(4)
Identify the weak diprotic acid.
A. HCOOH
B. H2CO3
C. H2SO4
D. CH3COOH
E. H3PO4 -ANSWER: H2CO3
Use the standard half-cell potentials listed below to calculate the standard cell potential for the following
reaction occurring in an electrochemical cell at 25°C. (The equation is balanced.)
3 Cl2(g) + 2 Fe(s) → 6 Cl-(aq) + 2 Fe3+(aq)
Cl2(g) + 2 e- → 2 Cl-(aq); E° = +1.36 V
Fe3+(aq) + 3 e- → Fe(s); E° = -0.04 V
,A. -1.32 V
B. +1.32 V
C. +4.16 V
D. +1.40 V
E. -1.40 V -ANSWER: +1.40 V
What is the pH of pure water at 40.0°C if the Kw at this temperature is 2.92 × 10^(-14)?
0.465
7.000
7.233
8.446
6.767 -ANSWER: 6.767
Given the following balanced equation, determine the rate of reaction with respect to [O2].
SO2(g)+O2(g)→2SO3(g)
A. Rate=+2Δ[O2]/Δt
B. Rate=+1/2(Δ[O2]/Δt)
C. Rate=−Δ[O2]/Δt
D. Rate=−1/2(Δ[O2]/Δt)
E. It is not possible to determine without more information. -ANSWER: Rate=−Δ[O2]/Δt
A reaction is followed and found to have a rate constant of 3.36 × 10^(4) M^(-1)s^(-1) at 344 K and a rate
constant of 7.69 M^(-1)s^(-1) at 219 K. Determine the activation energy for this reaction.
A. 42.0 kJ/mol
B. 11.5 kJ/mol
, C. 12.5 kJ/mol
D. 23.8 kJ/mol
E. 58.2 kJ/mol -ANSWER: 42.0 kJ/mol
Which of the following is a Brønsted-Lowry base?
A HCN
B CH4
C Cl2
D NH3
E None of the above are Brønsted-Lowry bases. -ANSWER: NH3
Determine the value of Kc for the following reaction if the equilibrium concentrations are as follows:
[N2]eq = 3.6 M, [O2]eq = 4.1 M, [N2O]eq = 3.3 × 10^(-18) M.
2 N2(g) + O2(g) ↔ 2 N2O(g)
2.0 × 10^(-37)
5.0 × 10^(36)
4.5 × 10^(18)
2.2 × 10^(-19)
4.9 × 10^(-17) -ANSWER: 2.0 × 10^(-37)
Which of the following acids will have the strongest conjugate base?
A. HClO4
B. HCN
C. HNO3
D. HI
E. HCl -ANSWER: HCN
CORRECT DETAILED ANSWERS LATEST UPDATE 2025
GRADED A+
For which reaction will Kp = Kc?
a. CaCO3 (s) ↔ CaO (s) + CO2 (g)
b. 2 H2O (l) ↔ 2 H2 (g) + O2 (g)
c. 2 HgO (s) ↔ Hg (l) + O2 (g)
d. S (s) + O2 (g) ↔ SO2 (g)
e. H2CO3 (s) ↔ H2O (l) + CO2 (g) -ANSWER: S (s) + O2 (g) ↔ SO2 (g)
For the following example, identify the following.
H2O (l) → H2O(g)
A.a positive ΔH and a positive ΔS
B. a positive ΔH and a negative ΔS
C. a negative ΔH and a positive ΔS
D. a negative ΔH and a negative ΔS
E. It is not possible to determine without more information. -ANSWER: a positive ΔH and a
positive ΔS
What is Δn for the following equation in relating Kc to Kp?
CH4(g) + H2O(g) ↔ CO(g) + 3 H2(g)
A. -1
B. -2
C. 3
,D. 1
E. 2 -ANSWER: 2
The reaction below has a Kp value of 41. What is the value of Kc for this reaction at 400 K?
N2(g) + 3 H2(g) ↔ 2 NH3(g)
A. 41
B. 4.4 × 10^(4)
C. 1.9 × 10^(4)
D. 2.4 × 10^(-2)
E. 2.3 × 10^(-5) -ANSWER: 4.4 × 10^(4)
Identify the weak diprotic acid.
A. HCOOH
B. H2CO3
C. H2SO4
D. CH3COOH
E. H3PO4 -ANSWER: H2CO3
Use the standard half-cell potentials listed below to calculate the standard cell potential for the following
reaction occurring in an electrochemical cell at 25°C. (The equation is balanced.)
3 Cl2(g) + 2 Fe(s) → 6 Cl-(aq) + 2 Fe3+(aq)
Cl2(g) + 2 e- → 2 Cl-(aq); E° = +1.36 V
Fe3+(aq) + 3 e- → Fe(s); E° = -0.04 V
,A. -1.32 V
B. +1.32 V
C. +4.16 V
D. +1.40 V
E. -1.40 V -ANSWER: +1.40 V
What is the pH of pure water at 40.0°C if the Kw at this temperature is 2.92 × 10^(-14)?
0.465
7.000
7.233
8.446
6.767 -ANSWER: 6.767
Given the following balanced equation, determine the rate of reaction with respect to [O2].
SO2(g)+O2(g)→2SO3(g)
A. Rate=+2Δ[O2]/Δt
B. Rate=+1/2(Δ[O2]/Δt)
C. Rate=−Δ[O2]/Δt
D. Rate=−1/2(Δ[O2]/Δt)
E. It is not possible to determine without more information. -ANSWER: Rate=−Δ[O2]/Δt
A reaction is followed and found to have a rate constant of 3.36 × 10^(4) M^(-1)s^(-1) at 344 K and a rate
constant of 7.69 M^(-1)s^(-1) at 219 K. Determine the activation energy for this reaction.
A. 42.0 kJ/mol
B. 11.5 kJ/mol
, C. 12.5 kJ/mol
D. 23.8 kJ/mol
E. 58.2 kJ/mol -ANSWER: 42.0 kJ/mol
Which of the following is a Brønsted-Lowry base?
A HCN
B CH4
C Cl2
D NH3
E None of the above are Brønsted-Lowry bases. -ANSWER: NH3
Determine the value of Kc for the following reaction if the equilibrium concentrations are as follows:
[N2]eq = 3.6 M, [O2]eq = 4.1 M, [N2O]eq = 3.3 × 10^(-18) M.
2 N2(g) + O2(g) ↔ 2 N2O(g)
2.0 × 10^(-37)
5.0 × 10^(36)
4.5 × 10^(18)
2.2 × 10^(-19)
4.9 × 10^(-17) -ANSWER: 2.0 × 10^(-37)
Which of the following acids will have the strongest conjugate base?
A. HClO4
B. HCN
C. HNO3
D. HI
E. HCl -ANSWER: HCN
